Answer : The values of all the quantum numbers for one electron in the 2p sublevel of a nitrogen (N) atom are, [tex](n=2,l=1,m_l=-1,0,+1,m_s=+\frac{1}{2}\text{ or }-\frac{1}{2})[/tex]
Explanation :
There are 4 quantum numbers :
Principle Quantum Numbers : It describes the size of the orbital. It is represented by n. n = 1,2,3,4....
Azimuthal Quantum Number : It describes the shape of the orbital. It is represented as 'l'. The value of l ranges from 0 to (n-1). For l = 0,1,2,3... the orbitals are s, p, d, f...
Magnetic Quantum Number : It describes the orientation of the orbitals. It is represented as [tex]m_l[/tex]. The value of this quantum number ranges from [tex](-l\text{ to }+l)[/tex]. When l = 2, the value of [tex]m_l[/tex] will be -2, -1, 0, +1, +2.
Spin Quantum number : It describes the direction of electron spin. This is represented as [tex]m_s[/tex] The value of this is [tex]+\frac{1}{2}[/tex] for upward spin and [tex]-\frac{1}{2}[/tex] for downward spin.
The electronic configuration of nitrogen atom is, [tex]1s^22s^22p^3[/tex]
Now we have to calculate the values of all the quantum numbers for one electron in the 2p sublevel of a nitrogen (N) atom.
For [tex]2p^1[/tex] :
[tex]n=2[/tex] (Because it is in 2nd shell)
[tex]l=1[/tex] (Because it is in 'p' orbital)
[tex]m_l=-1,0,+1[/tex] (Because l = 1)
[tex]m_s=+\frac{1}{2}\text{ or }-\frac{1}{2}[/tex] (Because of the sign convention)
Therefore, the values of all the quantum numbers for one electron in the 2p sublevel of a nitrogen (N) atom are, [tex](n=2,l=1,m_l=-1,0,+1,m_s=+\frac{1}{2}\text{ or }-\frac{1}{2})[/tex]
